What is the energy (kJ/mol) of the spectral line that corresponds to the transition of an electron from n = 6 to n = 2 in the He+ ion?
What is the energy (kJ/mol) of the spectral line that corresponds to the transition of an...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...
6. The first ionization energy of Au (IE1) is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom in the gas phase? Justify your answer with a calculation. 7. The energy of an electron in a hydrogen atom is -4.45 x 100 J. What energy level (n) does it occupy? Is there another valid energy level at -2.69 x 1020 ? If so, what is this other energy level? 8. What is the...
1. calculate the wavelength in nm of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level n=6 to the level n=2 2. with what max kinetic energy will electrons be ejected when this metal is exposed to light with a wavelength of 245nm? threshold frequency is 2.65*10^14 s^-1
Calculate the wavelength, in nanometers of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level n=7 to n=2?
1.. Suppose that you shine light of energy 1050 kJ/mol on an H atom in the ground state. What happens to the light and to the electron? Group of answer choices a. The light is not absorbed and the final energy of the electron is -1312 kJ/mol. b.. The light is absorbed and the final energy of the electron is −328 kJ/mol. c.. The light is not absorbed and the final energy of the electron is −1050 kJ/mol. d.. The...
Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level n = 3 to the level n = 2.
Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level n = 4 to the n = 2. nm
Electron Transitions and Spectral Lines Conceptual Question The spectrum of a hypothetical atom is shown in the figure.(Figure 1) Three distinct spectral series are shown, with the center series corresponding to transitions to a final state of n_f = 3. The indicated spectral line corresponds to the transition from an initial state of n_i =5 to the final state n_i = 3. Which of the lettered spectral lines corresponds to the transition from n_i = 6 to n_f = 3?...
2. Determine the ionization energy (in kJ mol-1) of a He+ ion with its electron in its lowest energy orbital.
Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level n=4 to the level n=1. λ=